2. Bonding

• Blue - HW
• Purple - attachments
• Red - important dates/quizzes/tests/exams
• Green - Text book reference
• Pink - Objectives being covered from the syllabus
• Turquoise - Labs

1. Introduction to bonding - covalent bonding and drawing Lewis Diagrams (structures or electron-dot diagrams)
2. HW: Finish practice sheet for homework - includes structures that do not obey the octet rule, and structures with multiple bonds.

1. Quiz - periodicity oxides(SL)/chlorides(HL both)
2. Cations and Anions
   1. Part A: testing for common ions in solution; developing a knowledge of precipitation as a test for identifying ions
   2. Part B: identifying cations and anions present in 4 solutions that are "unknown".
3. HW: preparation for PERIODICITY TEST next week.

1. Continuation of Lab: Part B: identifying cations and anions present in 4 solutions that are "unknown".
2. Tests for common gases - hydrogen, oxygen and carbon dioxide

1. Equations for the Cations & Anions Lab and going over the methodology. (Day 2)

1. Day off - thank you King Abdulla

1. Go over lab write up expectations.
2. VSEPR Theory - molecular shapes and bond angles.
3. Collect a handout from me and make notes during class.
4. You must have completed all the practice Lewis Structures (HW earlier)
5. 12 minute quiz this week - Lewis Structures, Molecular Shapes and Bond Angles Group 4 Project!!!
6. Lab write up - collecting and processing for the Cations/Anions Lab; Concluding for the 4 unknowns; Evaluation of your procedure for the 4 unknowns; As a separate lab: write a brief summary for the Common Gases - simply, what are the tests and what does a positive test give? Due: (Monday 7 March - Day 2); (Tuesday 15 March - Day 1).

1. Blue book p74 (Questions on p76 to think about, you can probably do them in your head)
2. Green book p101; shapes information p107-108 (SL) and p107-110 (HL)
3. HW: Green book: SL = 4.2 p106; HL = 14.1 p111 Due: Mar 12/13 (see instructions below)
4. Class work today: go over shapes and look at bond angles (180, 120, 109.5, 107, 104.5) (HL - 90 & 120 equatorial/axial positions); SL - using key words and phrases correctly EXPLAIN the shapes for molecules with up to 4 e pairs around the central atom; HL - do the same for molecules up to 6 e pairs around the central atom.
5. HW: priority over the other: SL explain all the shapes for the board; HL choose 2 for the SL set, 2 from the 5 e pair group and 1 from the 6 e pair group to explain the shapes for. Best examples will have both bonding pairs and non-bonding pairs in them. Due: next class (just try it!)

1. Answer the questions (even in pencil!) any way you like
2. Take a red pen and check the answers (you have them) - circle the errors and write a correction next to the error
3. Show me the completed work - I'm checking that you have done it and gone through these steps.

DO YOU WANT TO GET WORK DONE FASTER & UNDERSTAND IT???

1. YOU: Take good notes on top of the notes I give you in class WHILE IN CLASS - ask questions as we work WHILE IN CLASS
2. YOU: When you go home: just read the notes and have a wee think. If something doesn't make sense, use the text and just look for just that part (not the whole chapter....boring!!!) read the text and add in some notes to clarify the notes you took in class OR write your questions if it makes no sense; do it now while you are confused...the question will make more sense when you come and ask me [don't just come and say "I don't get it" - what about "it" don't you get?
3. US: Set aside one day a week when you bring some snacks and a drink - I'll put coffee on if it helps - and park up in the chemistry lab *3:15 - 4:00pm (Sunday a good day, it's before my meeting days and before the end-of-week quiz) and either have a list of questions we can blitz through or do your work and ask for questions as you need it. Use it as a day when you get the work done for chem and you can walk away with it done - no stress about taking 2 or 3 times longer at home alone trying to work it all out.
4. YOU: This option is for you to work with you and with me as needed - working with your friends is on your time - this is about you getting more out of YOUR WORK & FASTER.
5. AFTER SCHOOL TIME IS YOURS - *you only need to stay as long as you want to/until your work is done/until you have no questions/whatever - I'm just suggesting you slot the time in and have it there when you need it. Stay up to date - stay on the knowing side - feel like you're on top for change.

1. Going over examples done in the last class and the explanation of the shapes. Phrases like "bonding e pairs" and "non-bonding e pairs" need to be used correctly. Clear understanding that non-bonding pairs repel each other very strongly, non-bonding e pairs repel bonding e pairs strongly and that bonding e pairs repel each other in that order is important. It is the combination of all of these forces acting together that result in the final shape of a molecule.

1. You have a set of notes on polarity with very good images - keep those notes with your class notes.
2. revisit electronegativity and practice ordering which elements are more electronegative - work done from the whiteboard
3. notes from whiteboard on "pure covalent bonds", "polar covalent bonds" and "ionic bonds" - be very clear about ionic bonds being the result of oppositely charged ions NOT COVALENT BONDS!! Polarity is only a description of a type of COVALENT BOND.
4. Day two group: (Mar 9) we studied the relationship between bond number, length and strength - you have the paper.
5. Day one group: (Mar 12) also completed determining X,Y & Z and identifying types of bond work from the whiteboard.
6. HW: HL 14.1 green book p113 (there seems to be two exercise 14.1's??? but this one is on p 113 not p 111)

• Serious HL students: please see me about additional critical thinking questions for practice.
• Due dates are usually negotiated but once set the deadline is the deadline.

1. Revisit the relationship between number of bonds, length and strength (briefly)
2. Complete polarity work from the whiteboard - determine X, Y & Z and identify the type of bond
3. Check 4.2 and 14.1 p111 completion - HW 14.1 p 113

1. As above
2. Overview all covalent work 4.2; metallic bonding 4.4; ionic bonding 4.1

1. 8 - 12 minute quiz on Lewis structures, molecular shapes (bond angles) and polarity. You can expect 3 structures and some explaining to do.

1. What is structure? What is the bonding?
2. What are the examples of properties we have been learning about?
3. How does the structure and the bonding result in the properties?
4. How do I explain these clearly?
5. Am I a good student?

1. Let's take a look at the topic checklist (you have it - now look at it) - 4.5 is the aspect to keep your eyes on - it's the really important part.
2. Whiteboard notes: COMPARE the nature of ionic, covalent and metallic bonding - they are all electrostatic but they are all different at the same time. DISCUSS the properties (different types of properties) using KNOWLEDGE about the structure and bonding. Eg Solid metal conducts electricity but solid diamond does not. Solid metal has mobile "delocalised" electrons throughout the 3D network of cations. When a potential difference (electricity) is applied to the metal the delocalised electrons will carry the charge. Diamond is a 3D network of covalently bonded atoms. The electrons in the bonds are localised and not available to carry any charge when a potential difference is applied. Could you say that?
3. HW:Practice questions given out and to be completed. These are the sorts of questions you can expect so DO THEM.

1. Intermolecular forces - van der Waals' forces, dipole-dipole and hydrogen bonding see page 78.
2. The question sheet with 1-12 on it should be finished.
3. The "Solid Summary" needs to almost be done.

1. SL have finished. You have practice work to complete, check (using red pen and making corrections) then show me so I record your completion.
2. HL - Hybridisation of orbitals, and bond overlap theory. You have powerpoint notes. Question sheet for practice.

1. Recap hybridisation.
2. Sigma and Pi bonds. Internuclear axis, shapes of orbitals (s and p), multiple bonds and resonance using nitrate and benzene examples.